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Chapter 10 Gases John Bookstaver St. Charles Community College Cottleville, MO Chemistry, The Central Science , 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten
Characteristics of Gases ,[object Object],[object Object],[object Object],[object Object]
[object Object],Pressure ,[object Object],P  = F A
Units of Pressure ,[object Object],[object Object],[object Object],[object Object]
Units of Pressure ,[object Object],[object Object],[object Object],[object Object]
Manometer ,[object Object]
Standard Pressure ,[object Object],[object Object],[object Object],[object Object],[object Object]
Boyle’s Law ,[object Object]
As  P  and  V  are inversely proportional ,[object Object],[object Object],[object Object],[object Object],PV  =  k
Charles’s Law ,[object Object],A plot of  V  versus  T  will be a straight line. ,[object Object],V T =  k
Avogadro’s Law ,[object Object],[object Object],V  =  kn
Ideal-Gas Equation ,[object Object],[object Object],[object Object],[object Object],[object Object],V    nT P
Ideal-Gas Equation ,[object Object]
Ideal-Gas Equation ,[object Object],then becomes or PV  =  nRT nT P V    nT P V  =  R
Densities of Gases ,[object Object],n V P RT =
[object Object],[object Object],Densities of Gases ,[object Object],n        =  m P  RT m V =
Densities of Gases ,[object Object],[object Object],Note:  One only needs to know the molecular mass, the pressure, and the temperature to calculate the density of a gas. P  RT m V = d  =
Molecular Mass ,[object Object],Becomes P  RT d  = dRT P    =
Dalton’s Law of Partial Pressures ,[object Object],[object Object],[object Object]
Partial Pressures ,[object Object],[object Object]
Kinetic-Molecular Theory ,[object Object]
Main Tenets of Kinetic-Molecular Theory ,[object Object]
Main Tenets of Kinetic-Molecular Theory ,[object Object]
Main Tenets of Kinetic-Molecular Theory ,[object Object]
Main Tenets of Kinetic-Molecular Theory ,[object Object]
Main Tenets of Kinetic-Molecular Theory ,[object Object]
Effusion ,[object Object]
Effusion ,[object Object]
Diffusion ,[object Object]
Graham's Law KE 1 KE 2 = 1/2  m 1 v 1 2 1/2  m 2 v 2 2 = = m 1 m 2 v 2 2 v 1 2  m 1  m 2  v 2 2  v 1 2 = v 2 v 1 =
Real Gases ,[object Object]
Real Gases ,[object Object]
Deviations from Ideal Behavior ,[object Object]
Corrections for Nonideal Behavior ,[object Object],[object Object]
The van der Waals Equation ) ( V   −   nb ) =  nRT n 2 a V 2 ( P  +

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Ch10 outline

  • 1. Chapter 10 Gases John Bookstaver St. Charles Community College Cottleville, MO Chemistry, The Central Science , 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten
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  • 30. Graham's Law KE 1 KE 2 = 1/2 m 1 v 1 2 1/2 m 2 v 2 2 = = m 1 m 2 v 2 2 v 1 2  m 1  m 2  v 2 2  v 1 2 = v 2 v 1 =
  • 31.
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  • 35. The van der Waals Equation ) ( V − nb ) = nRT n 2 a V 2 ( P +